Question 1

Identify each of the following molecular orbitals.

Accepted Answer

The answer of Identify each of the following molecular orbitals....

Question 2

Molecular orbital theory can be applied ________

Accepted Answer

A) only to two adjacent metal atoms. 
B) only to a few metal atoms that are very close to each other. 
C) to any number of metal atoms. 
D) to nonmetals only, not to metals. 
E) to nonmetals and ionic bonds only, not to metals. 
A) only to two adjacent metal atoms. 
B) only to a few metal atoms that are very close to each other. 
C) to any number of metal atoms. 
D) to nonmetals only, not to metals. 
E) to nonmetals and ionic bonds only, not to metals.

Question 3

Consider the molecule below-how many sp hybridized carbon atoms are present in the molecule?

Accepted Answer

A) 2 
B) 0 
C) 3 
D) 4 
E) 1 
A) 2 
B) 0 
C) 3 
D) 4 
E) 1

Question 4

Which one of the following statements regarding molecular orbital theory is correct?

Accepted Answer

A) Two bonding orbitals and two antibonding orbitals are formed from one atomic orbital on each of two atoms. 
B) p atomic orbitals cannot form F1F1F1S1F1F1F10molecular orbitals. 
C) A 2s F1F1F1S1F1F1F10 orbital has a higher energy than a 2s F1F1F1S1F1F1F10* orbital. 
D) Only F1F1F1S1F1F1F10molecular orbitals can be formed from p atomic orbitals. 
E) s atomic orbitals can only form F1F1F1S1F1F1F10molecular orbitals. 
A) Two bonding orbitals and two antibonding orbitals are formed from one atomic orbital on each of two atoms. 
B) p atomic orbitals cannot form F1F1F1S1F1F1F10molecular orbitals. 
C) A 2s F1F1F1S1F1F1F10 orbital has a higher energy than a 2s F1F1F1S1F1F1F10* orbital. 
D) Only F1F1F1S1F1F1F10molecular orbitals can be formed from p atomic orbitals. 
E) s atomic orbitals can only form F1F1F1S1F1F1F10molecular orbitals.

Question 5

When Ge is doped with Ga, it produces a(n) ________-type semiconductor.

Accepted Answer

A) p 
B) n 
C) q 
D) np 
E) No semiconductor will be produced. 
A) p 
B) n 
C) q 
D) np 
E) No semiconductor will be produced.

Question 6

What is the hybridization of the iodine atom in ICl3?

Accepted Answer

A) sp2 
B) sp3d2 
C) sp3d 
D) sp3 
E) sp 
A) sp2 
B) sp3d2 
C) sp3d 
D) sp3 
E) sp

Question 7

Which of these molecules do not have a dipole moment?

Accepted Answer

A) PCl5 and SiCl4 
B) POCl3, SO2Cl2, and SO3 
C) POCl3 and SO2Cl2 
D) PCl5, POCl3, SOCl2, SO3, and SiCl4 
E) PCl5, SF6, SO3, and SiCl4 
A) PCl5 and SiCl4 
B) POCl3, SO2Cl2, and SO3 
C) POCl3 and SO2Cl2 
D) PCl5, POCl3, SOCl2, SO3, and SiCl4 
E) PCl5, SF6, SO3, and SiCl4

Question 8

The correct H-N-H bond angle in NH3 is ________

Accepted Answer

A) the same as the H-O-H angle in water. 
B) exactly 109.5F1F1F1S1F1F1F10. 
C) greater than 109.5F1F1F1S1F1F1F10. 
D) less than 109.5F1F1F1S1F1F1F10. 
E) 120F1F1F1S1F1F1F10. 
A) the same as the H-O-H angle in water. 
B) exactly 109.5F1F1F1S1F1F1F10. 
C) greater than 109.5F1F1F1S1F1F1F10. 
D) less than 109.5F1F1F1S1F1F1F10. 
E) 120F1F1F1S1F1F1F10.

Question 9

Which of the following molecules has a bond order that is less than one?

Accepted Answer

A) F2 
B) He2F1F1F1S1F1F1F10 
C) Ne22F1F1F1S1F1F1F10 
D) N2 
E) O22F1F1F1S1F1F1F10 
A) F2 
B) He2F1F1F1S1F1F1F10 
C) Ne22F1F1F1S1F1F1F10 
D) N2 
E) O22F1F1F1S1F1F1F10

Question 10

Which of these molecules have a dipole moment?

Accepted Answer

A) PCl5 and SiCl4 
B) POCl3, SO2Cl2, and SO3 
C) POCl3 and SO2Cl2 
D) PCl5, POCl3, SOCl2, SO3, and SiCl4 
E) PCl5, SF6, SO3, and SiCl4 
A) PCl5 and SiCl4 
B) POCl3, SO2Cl2, and SO3 
C) POCl3 and SO2Cl2 
D) PCl5, POCl3, SOCl2, SO3, and SiCl4 
E) PCl5, SF6, SO3, and SiCl4

Question 11

Which of these molecules is chiral?

Accepted Answer

A) I and II 
B) I and III 
C) I and IV 
D) II and III 
E) II and IV 
A) I and II 
B) I and III 
C) I and IV 
D) II and III 
E) II and IV

Question 12

Predict the bond order of the NOF1F1F1S1F1F1F10 molecular ion.

Accepted Answer

A) 2 
B) 2.5 
C) 3 
D) 1 
E) 1.5 
A) 2 
B) 2.5 
C) 3 
D) 1 
E) 1.5

Question 13

Which of the following statements about bonds between two carbon atoms is/are correct? (I) Bond strength increases as more electrons are shared between the atoms.
(II) Bond strength increases as the overlap between atomic orbitals increases.
(III) Hybrid orbitals are used to describe (account for) the geometry (bond angles) around each carbon atom.

Accepted Answer

A) I 
B) II 
C) III 
D) Only two of these are correct statements. 
E) All three are correct statements. 
A) I 
B) II 
C) III 
D) Only two of these are correct statements. 
E) All three are correct statements.

Question 14

Identify the polar molecule.

Accepted Answer

A) CF4 
B) SiH4 
C) CHCl3 
D) CS2 
E) CO2 
A) CF4 
B) SiH4 
C) CHCl3 
D) CS2 
E) CO2

Question 15

Which bond is the least polar?

Accepted Answer

A) H-C 
B) H-N 
C) H-O 
D) H-Cl 
E) H-F 
A) H-C 
B) H-N 
C) H-O 
D) H-Cl 
E) H-F

Question 16

Which bond angle is the smallest?

Accepted Answer

A) H-C-H in CH4 
B) H-C-H in C2H4 
C) H-C-H in H2CO 
D) H-C-C in C2H2 
E) H-C-O in H2CO 
A) H-C-H in CH4 
B) H-C-H in C2H4 
C) H-C-H in H2CO 
D) H-C-C in C2H2 
E) H-C-O in H2CO

Question 17

What is the valence electron molecular orbital electron configuration of N2?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 18

Predict the indicated bond angles (less than, exactly, or greater than) in each of the following molecules.

Accepted Answer

@#IMG-DLM& Greater than 90° Le

Question 19

What is the molecular geometry of SF4?

Accepted Answer

A) tetrahedral 
B) square pyramidal 
C) seesaw 
D) square planar 
E) T-shaped 
A) tetrahedral 
B) square pyramidal 
C) seesaw 
D) square planar 
E) T-shaped

Question 20

Which statement regarding a F1F1F1S1F1F1F10 bond between two carbon atoms is correct?

Accepted Answer

A) The region of high electron density lies along the bond axis connecting the nuclei of the two atoms. 
B) The bond can be described by the overlap of sp hybrid orbitals from each atom. 
C) The bond can be described by the overlap of sp2 hybrid orbitals from each atom. 
D) The bond can be described by the overlap of p atomic orbitals from each atom. 
E) The bond can be described by the overlap of a p atomic orbital from one atom with an sp2 hybrid orbital from the other atom. 
A) The region of high electron density lies along the bond axis connecting the nuclei of the two atoms. 
B) The bond can be described by the overlap of sp hybrid orbitals from each atom. 
C) The bond can be described by the overlap of sp2 hybrid orbitals from each atom. 
D) The bond can be described by the overlap of p atomic orbitals from each atom. 
E) The bond can be described by the overlap of a p atomic orbital from one atom with an sp2 hybrid orbital from the other atom.

Exam 9: Molecular Geometry: Shape Determines Function

Identify each of the following molecular orbitals.

Molecular orbital theory can be applied ________

Consider the molecule below-how many sp hybridized carbon atoms are present in the molecule?

Which one of the following statements regarding molecular orbital theory is correct?

When Ge is doped with Ga, it produces a(n) ________-type semiconductor.

What is the hybridization of the iodine atom in ICl3?

Which of these molecules do not have a dipole moment?

The correct H-N-H bond angle in NH3 is ________

Which of the following molecules has a bond order that is less than one?

Which of these molecules have a dipole moment?

Which of these molecules is chiral?

Predict the bond order of the NO molecular ion.

Identify the polar molecule.

Which bond is the least polar?

Which bond angle is the smallest?

What is the valence electron molecular orbital electron configuration of N2?

Predict the indicated bond angles (less than, exactly, or greater than) in each of the following molecules.

What is the molecular geometry of SF4?

Which statement regarding a  bond between two carbon atoms is correct?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

What is the hybridization of the iodine atom in ICl₃?

The correct H-N-H bond angle in NH₃ is ________

Predict the bond order of the NO^ molecular ion.

What is the valence electron molecular orbital electron configuration of N₂?

What is the molecular geometry of SF₄?